Question

Write the cell representation and calculate equilibrium constant for the following redox reaction :
`Ni_((s))+2Ag_((aq))^(+)(1M) to Ni_((aq))^(2+)(1M) to 2Ag_((s)) at 25^(@)C`
`E_(Ni)^_(Ni)^(2+)(@)=0*25V and E_(Ag)(+) ^(@)=0*799V`

Answer 1

`Ni_((1M))^(2+)//Ni||Ag^(+)(1M)||Ag`
`E_("cell")^(@)=(0*0592)/(n)log_(10)K`
`E_("Cell")^(@)=E_(Ag)^(@)-E_(Ni)^(@)`
`=0*799(V)-(-0*25)=1*049V`
`:. =1*048=(0*0592)/(2)log_(10)K`
`1*049=(0*0592)/(2)log_(10)K`
`log_(10)K=(1*049xx2)/(0*0592)`
`=35*44`
`K="antilog"=35*4=2*754xx10^(23)`